Electron Shielding: Understanding the Role of Orbital Repulsion

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SUMMARY

This discussion focuses on electron shielding and its relationship with orbital repulsion, particularly in the context of effective nuclear charge (Z). Participants confirm that inner electrons shield outer electrons from the nuclear charge, affecting properties like electronegativity and ionization energy. The conversation highlights the significance of understanding electron configuration, especially in transition elements where shielding effects are pronounced. The discussion also critiques the generalizations found in textbooks regarding these concepts.

PREREQUISITES
  • Understanding of effective nuclear charge (Z)
  • Knowledge of electron configuration and orbital filling
  • Familiarity with periodic trends, particularly electronegativity
  • Basic concepts of ionization energy and its relation to electron shielding
NEXT STEPS
  • Research the concept of electron shielding in transition metals
  • Study the relationship between electronegativity and atomic structure
  • Explore detailed resources on effective nuclear charge (Z) calculations
  • Examine the role of orbital repulsion in chemical bonding
USEFUL FOR

Chemistry students, educators, and anyone interested in atomic structure and periodic trends will benefit from this discussion, particularly those seeking a deeper understanding of electron shielding and its implications in chemical properties.

Bladibla
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Now this relates to the berylium + Lithium thread i made earlier.. (although not entierly)

Is electron 'shielding' due to replusion between electron orbitals?

http://facultyfp.salisbury.edu/dfrieck/htdocs/212/rev/zeff/shielding.htm

I've had a look at this site, but in somewhat generalizes too much for me. Therfore, can i presume the electrons which occupy the 'inner' orbitals cancel out some of the values of the nuclear charge?
 
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You need to read up more on the topic of effective nuclear charge (Z). Browse through the index of your text.

Why does electronegativity increase as you move across a specific row of the periodict table?
 
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Ill certainly do that, however, it seems to me the textbooks i have (provided from school) generalizes too much, just saying 'electron shielding causes lower ionisation energy...etc'

I just got a new book (which seems good) so ill read through it, however, it would be appreciative to have one here..
 
Bladibla said:
...Therfore, can i presume the electrons which occupy the 'inner' orbitals cancel out some of the values of the nuclear charge?

Roughly speaking, yes, that is what shielding is. The inner electrons "shield" the outer electrons from the field due to the nucleus.
 
It happens in transition elements more often than in main group elements. Basically since electrons fill in the 4s orbital before the 3d the new 3d electrons shield the 4s orbital from the nuclear charge of the nucleus as they are in a lower energy orbital and thus between the 4s orbital and the nucleus. Also I am really drunk so if something was omitted or factually incorrect my bad.
 

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